On phosphoric acid conjugated base
phosphoric acid, the nature of its conjugated base is related to many chemical changes. Phosphoric acid ($H_3PO_3 $), deproton ($H ^ + $), becomes its conjugated base.

The structure of phosphoric acid has a dihydroxy group connected to phosphorus, and a double bond between oxygen and phosphorus. When it deprotons, the hydrogen of the hydroxyl group is easily separated, and the resulting conjugated base has a different charge distribution. The stability of this conjugated base is restricted by many factors.

The electron effect is one of them. The electron cloud density of the phosphorus atom varies due to the electron-absorbing property of the oxygen atom. In a conjugated base, the negative charge can be dispersed through the oxygen atom to stabilize it. The resonance effect is also heavy. The conjugated base can store a resonance structure, so that the negative charge can be dispersed in different atoms, increasing its stability.

Furthermore, the solvent effect cannot be ignored. In polar solvents, the solvent interacts with the conjugated base, or stabilizes or destabilizes the conjugated base. Water is a common solvent, and water molecules can form hydrogen bonds with the conjugated base, affecting its properties.

Phosphite conjugated base is often an active species in chemical reactions. In acid-base reactions, it can be used as a base to bind with protons. In redox reactions, because of its structure and electronic properties, or participate in electron transfer.

In short, the properties of phosphite conjugated bases are of deep significance in the field of chemistry, from structure to reaction, and are essential for chemical study and application.